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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

9. Quantum Mechanics

Bohr Equation

General Chemistry

9. Quantum Mechanics

Bohr Equation

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Multiple Choice

For hydrogen, what is the wavelength of the photon emitted when an electron drops from the n=3 level to the n=2 level? The Rydberg constant is 1.097 × 10^7 m^-1.

486 nm

410 nm

434 nm

656 nm

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Verified step by step guidance

Understand that the problem involves calculating the wavelength of a photon emitted during an electron transition in a hydrogen atom. This is done using the Rydberg formula for hydrogen.

The Rydberg formula is given by:

\frac{1}{λ} = R (\frac{1}{n^{1}} - \frac{1}{n^{2}})

, where

λ

is the wavelength,

R

is the Rydberg constant, and

n

are the principal quantum numbers of the initial and final energy levels.

Identify the values for the quantum numbers:

n_{1}

is 2 and

n_{2}

is 3. Substitute these values into the Rydberg formula.

Substitute the Rydberg constant value

R = 1.097 \times 10^{7} m - 1

into the formula.

Solve for

λ

by calculating the difference in the reciprocals of the squares of the quantum numbers, then take the reciprocal of the result to find the wavelength in meters, and convert it to nanometers.